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Ácido y Base.
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Ácido y Base. (Ácido y Base.)
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Ácido-BaseÁcido-Base.
1. Diluciones electrolíticas.
Son muy estables, reversibles y conducen la electricidad.
Soluto disuelve en un disolvente y se disocia en iones. El soluto puede ser ácido o base.
𝑁𝑎𝐶𝑙 ↔ 𝑁𝑎+ + 𝐶𝑙 −
A) Arrhenius (1884).
Ácido: Sustancia eléctricamente neutra que en disolución acuosa forma protones (𝐻 +
hidrón).
𝐻𝐶𝑙 → 𝐻+ + 𝐶𝑙 −
𝐶𝐻3𝐶𝑂𝑂𝐻 → 𝐶𝐻3𝐶𝑂𝑂 − + 𝐻+
Base: Sustancia eléctricamente neutra que en disolución acuosa forma anión hidróxido
(𝑂𝐻 − ).
𝑁𝑎𝑂𝐻 → 𝑁𝑎+ + 𝑂𝐻−
Excepciones: Solo en disolución acuosa y BF3 -ácido y NH3-Base.
B) Bronsted-Lowry (1924).
Ácido: Cualquier especie química capaz de ceder protones a otra sustancia.
𝐶𝐻3𝐶𝑂𝑂𝐻 + 𝐻2𝑂 → 𝐶𝐻3𝐶𝑂𝑂 − + 𝐻3𝑂 +
Ácido 1 Base 2 Base conjugada 1 Ácido conjugado 2
Ácido conjugado: Especie química resultante tras capturar 𝐻+
Base conjugada: Especie química que resulta tras ceder un 𝐻+ del ácido.
C) Lewis (1923):
Ácido es capaz de aceptar y compartir un par de electrones.
BF3:
Base: Capaz de ceder y compartir un par de electrones.
NH3:
D) Grado de disociación.
Ácidos y bases se disocian pero no todos lo hacen con la misma intensidad.
Se disocian completamente: Ácidos y bases fuertes.
𝐻𝐶𝐿 ↔ 𝐶𝑙 − + 𝐻 +
HCL 𝐶𝑙 − + 𝐻+
Inicial 1 mol 0 0
Reacción -1 mol 1 mol 1mol
Equilibrio 0 1 mol 1mol
𝑛º 𝑚𝑜𝑙𝑒𝑠 𝑞𝑢𝑒 𝑠𝑒 𝑑𝑖𝑠𝑜𝑐𝑖𝑎𝑛 1𝑚𝑜𝑙
𝛼= 𝑛º 𝑚𝑜𝑙𝑒𝑠 𝑖𝑛𝑖𝑐𝑖𝑎𝑙𝑒𝑠.
; 𝛼 = 1𝑚𝑜𝑙 = 1 ; 𝛼% = 1 ∗ 100 = 100
No se disocian completamente: Ácidos y bases débiles.
𝐶𝐻3𝐶𝑂𝑂𝐻 ↔ 𝐶𝐻3𝐶𝑂𝑂 − + 𝐻 +
CH3COOH 𝐶𝐻3𝐶𝑂𝑂 − + 𝐻+
Inicial 1 mol 0 0
Reacción -0,3mol 0,3mol 0,3mol
Equilibrio 0,7 0,3 mol 0,3mol
𝑛º 𝑚𝑜𝑙𝑒𝑠 𝑞𝑢𝑒 𝑠𝑒 𝑑𝑖𝑠𝑜𝑐𝑖𝑎𝑛 0,3𝑚𝑜𝑙
𝛼= ;𝛼 = = 0,3 ; 𝛼% = 0,3 ∗ 100 = 30% 𝑑𝑖𝑠𝑜𝑐𝑖𝑎𝑑𝑜
𝑛º 𝑚𝑜𝑙𝑒𝑠 𝑖𝑛𝑖𝑐𝑖𝑎𝑙𝑒𝑠. 1𝑚𝑜𝑙
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